nuclear chemistry element# of neutrons # of protons # of electrons atomic # mass # scan- dium iron n...

NUCLEAR CHEMISTRY

Element # of neutrons

# of protons

# of electrons

Atomic#

Mass #

Scan-dium

Iron

Fill in the chart below.Fill in the chart below.

452124 2121

542628 2626

ATOMIC STRUCTURE REVIEW

• Nuclear chemistry is the study of the structure of atomic nuclei and the changes they undergo.

Nuclear Chemistry

Nuclear Reactions

• There are three different types of nuclear reactions: radioactive decay, fission, and fusion.

Radioactive Decay

• Unstable nuclei spontaneously emit radiation to attain more stable atomic configurations.

• Radioactive decay is a type of nuclear reaction which involves atoms that undergo radioactive (alpha, beta, and gamma) decay.

• During radioactive decay, unstable atoms lose energy by emitting one of several types of radiation.

Radioactive Decay

• Nuclear decay is a random event.

• This is very much like popping popcorn. When we pour popcorn kernels into a popcorn popper, there is no way to know which kernel will pop first. And once that first kernel pops, it will never be a kernel again...it is forever changed!

Radioactive Decay

Types of Radiation

• The three most common types of radiation are alpha (α), beta (β), and gamma (γ).

Name Symbol Formula Mass Charge Description

β

α

γ high energy radiation

Types of Radiation

alpha

beta

gamma

high speed electrons

helium nuclei

4 +2

0

0

0

-1

He42

0

-1e

Alpha

• The charge of an alpha particle is 2+ due to the presence of the two protons.

• An alpha particle (α) has the same composition as a helium nucleus—two protons and two neutrons—and is therefore given the symbol .

• Because of their mass and charge, alpha particles are relatively slow-moving compared with other types of radiation.

• Thus, alpha particles are not very penetrating—a single sheet of paper stops alpha particles.

Alpha

Beta

• A beta particle is a very-fast moving electron that has been emitted from a neutron of an unstable nucleus.

• Beta particles are represented by the symbol

The zero superscript indicates the insignificant mass of an electron in comparison with the mass of a nucleus.

• The –1 subscript denotes the negative charge of the particle.

• Beta radiation consists of a stream of fast-moving electrons.

Beta

• Because beta particles are both lightweight and fast moving, they have greater penetrating power than alpha particles.

• A thin metal foil is required to stop beta particles.

Beta

Gamma

• As you can see from the symbol, both the subscript and superscript are zeroes.

• Gamma rays are high-energy (short wavelength) electromagnetic radiation. They are denoted by the symbol .

• Thus, the emission of gamma rays does not change the atomic number or mass number of a nucleus.

Gamma

• Gamma rays are the most penetrating.

• Concrete, lead, or steel must be used to block gamma rays.

Gamma

Radiation

Alpha, Beta or Gamma?

??

??

??

Types of Radiation

??

??

??

Types of Radiation

• Negatively charged beta particles are deflected toward the positively charged plate.

??

??

Types of Radiation

• Positively charged alpha particles are deflected toward the negatively charged plate.

??

Types of Radiation

• Gamma rays, which have no electrical charge, are not deflected.

Types of Radiation

• In an electric or magnetic field, alpha particles are deflected less than beta rays because they are more massive.

• Radioactive nuclei undergo decay in order to gain stability.

Nuclear Stability

• All elements with atomic numbers greater than 83 are radioactive.

Balancing a Nuclear Equation

• Nuclear equations are used to show nuclear transformations.

• Balanced nuclear equations require that both the atomic number and the mass number must be balanced.

XA

Z

Atomic number

Mass number

Element symbol


XZ

A

1. When beryllium-9 is bombarded with alpha particles (helium nuclei), a neutron is produced. The balanced nuclear reaction is given as:

Be + He n +94

42

10

???


• On the reactant side, the mass numbers equal (9 + 4) = 13.

Be + He n +94

42

10

???


• On the product side, the mass number equals 1.

• The product side needs an additional 12 for the mass number.

12

• On the reactant side, the atomic numbers equal (4 + 2) = 6.

Be + He n +94

42

10


• On the product side, the atomic number equals 0.

• The product side needs an additional 6 for the atomic number.

126

• The atomic number (the number on the bottom) determines the identity of the element.

Be + He n +94

42

10


12 6

Be + He n +94

42

10


12 6

• The element with an atomic number of 6 is carbon.

C

2. When nitrogen-14 is bombarded with a neutron, a proton is produced. The balanced nuclear equation can be written as:

N + n p +147

10

11

???


• On the reactant side, the mass numbers equal (14 + 1) = 15.


• On the product side, the mass number equals 1.

• The product side needs an additional 14 for the mass number.

N + n p +147

10

11

???14

• On the reactant side, the atomic numbers equal (7 + 0) = 7.


• On the product side, the atomic number equals 1.

• The product side needs an additional 6 for the atomic number.

N + n p + 147

10

11

14 6

• The atomic number (the number on the bottom) determines the identity of the element.

N + n p +147

10

11


14 6

N + n p +147

10

11


14 6

• The element with an atomic number of 6 is carbon.

C

Th He + 230 90

42


226 88

3. Thorium-230 undergoes alpha decay.

Ra???

U He +234 92

42


230 90 Th???

4. Uranium-234 undergoes alpha decay.

Co e + 5027

0-1


50 28

Ni???

5. Cobalt-50 undergoes beta decay.

Question 6

What element is formed when undergoes beta decay? Give the atomic number and mass number of the element.

Question 7

Write a balanced nuclear equation for the alpha decay of the following radioisotope.

231235U He + Th9092

42

Question 8

Nitrogen-12 decays into a positron and another element. Write the balanced nuclear equation.

N e + C 12 7

12

6 0 1

Question 9

Uranium-238 is bombarded with a neutron. One product forms along with gamma radiation. Write the balanced nuclear equation.

U + n U + γ238 92

1 0

239 92

Question 10

Nitrogen-14 is bombarded with deuterium (hydrogen-2). One product forms along with an alpha particle. Write the balanced nuclear equation.

N + H C + He14 7

2 1

12 6

42

STOP HERE

Element # of neutrons

# of protons

# of electrons

Atomic#

Mass #

Pc

Xv

Fill in the chart below. All elements Fill in the chart below. All elements are imaginary so DO NOT USE a are imaginary so DO NOT USE a periodic table.periodic table.

582830 2828

1015348 5353

ATOMIC STRUCTURE REVIEW

How many moles of aluminum are How many moles of aluminum are 56.7 grams of aluminum?56.7 grams of aluminum?

56.7 grams Al56.7 grams Al

grams Algrams Al

mole Almole Al

27.027.0

11__

__

(2.10)

grams Algrams Al

MOLE CONVERSION REVIEW

How many formula units of NaCl are How many formula units of NaCl are in 0.0594 moles of NaCl?in 0.0594 moles of NaCl?

0.0594 moles NaCl0.0594 moles NaCl

mole NaClmole NaCl

f. Units NaClf. Units NaCl

1

6.022 x 106.022 x 102323

__

_

(3.58 x 1022)

f. units NaClf. units NaCl

MOLE CONVERSION REVIEW

• Balance the following nuclear equation with the missing particle.

NUCLEAR EQUATIONS REVIEW

___42

23994 HePu U235

92

• Balance the following nuclear equation with the missing particle.


___3015

42

2713 PHeAl n10

• Balance the following nuclear equation with the missing number.


nYInU 10

9539

13953

10

23592 __ 2

• A half-life is the time required for one-half of a radioisotope’s nuclei to decay into its products.

• Radioactive decay rates are measured in half-lives.

Radioactive Decay Rates

• For example, the half-life of the radioisotope strontium-90 is 29 years.

• If you had 10.0 g of strontium-90 today, 29 years from now you would have 5.0 g left.

• The decay continues until negligible strontium-90 remains.



• The graph shows the percent of a stontium-90 sample remaining over a period of four half-lives.

• With the passing of each half-life, half of the strontium-90 sample decays.

• Chemical reaction rates are greatly affected by changes in temperature, pressure, and concentration, and by the presence of a catalyst.

• In contrast, nuclear reaction rates remain constant regardless of such changes.

• In fact, the half-life of any particular radioisotope is constant.



time amount

0 Initial amount

Half-life Initial amount ÷ 2

Half-life x 2 Initial amount ÷ 4



Calculating Amount of Remaining Isotope

11. Iron-59 is used in medicine to diagnose blood circulation disorders. The half-life of iron-59 is 44.5 days. How much of a 2.000-mg sample will remain after 133.5 days?

11. Iron-59 is used in medicine to diagnose blood circulation disorders. The half-life of iron-59 is 44.5 days. How much of a 2.000-mg sample will remain after 133.5 days?

(0.250 mg)

Time (days)Time (days) Amount (mg)Amount (mg)

0 2.000

44.5

See if the problem tells you

the starting amount.

See if the problem tells you the half-life time.

Did the problem give you the final time or

final amount?

89

133.5

Now cut the

amount in half for

each row.1.000

0.500

0.250

Take the half-life

time and multiply it by 2, then by 3, etc. to get the total time.

Question

12. Cobalt-60 has a half-life of 5.27 years. How much of a 10.0 g sample will remain after 21.08 years?

(0.625 g)

Question

13. If 100.0 g of carbon-14 decays until only 25.0 g of carbon is left after 11,460 yr, what is the half-life of carbon-14?

13. If 100.0 g of carbon-14 decays until only 25.0 g of carbon is left after 11,460 yr, what is the half-life of carbon-14?

(5730 yr)

Time (yr)Time (yr) Amount (g)Amount (g)

0 100.0




Now see if the

problem tells you the final amount or final time.

11,460

Since you have the

starting mass and final

mass, cut the amount in half for each row

until you reach the final

amount.

50.0

25.0

This problem does not.

Input the time that

corresponds with the final

amount.

Take the total time and divide

by the number of times you

cut the mass in half.

11,460 / 2

This problem tells you BOTH, the final amount and final

time.

Question

14. What is the half-life in days of an isotope if 125 grams of a 1000 gram sample remain after 15 days?

(5 days)

Question

15. What is the half-life in years of an isotope if 1 gram of a 16 gram sample remains after 16 years?

(4 years)

Question

16. The half-life of hafnium-156 is 0.025 s. How long will it take a 560 g sample to decay to one-fourth its original mass?

16. The half-life of hafnium-156 is 0.025 s. How long will it take a 560 g sample to decay to one-fourth its original mass?

(0.050 s)

timetime amountamount

0 560

0.025




See if the problem tells you the final amount.

0.050

Now cut the

amount in half for

each row until you reach the

final amount.

280

¼ (560) = 140

Now double the time for each used

row.

Question

17. Chromium-48 has a short half-life of 21.6 h. How long will it take 360.00 g of chromium-48 to decay to 11.25 g?

(108 h)

Question

18. If the half-life of uranium-235 is 7.04 x 108 yr and 12.5 g of uranium-235 remain after 28.2 x 108 yr, how much of the radioactive isotope was in the original sample?

(200 g)

Question

19. Carbon-14 has a half-life of 5730 years. How much of a 250. g sample will remain after 5730 years?

(125 g)

Nuclear Reactions

• A second type of nuclear reaction is fission.

• The basic difference in radioactive decay and fission is that in radioactive decay, an unstable isotope spontaneously undergoes a nuclear change.

Nuclear Reactions

• In nuclear fission, a fissionable isotope absorbs a neutron, becomes unstable, and then fissions by breaking into a couple of pieces and releasing one or more neutrons plus a large amount of energy.

• Nuclear fission is usually thought of as intentionally caused.

Nuclear Fission

• Heavy atoms (mass number > 60) tend to break into smaller atoms, thereby increasing their stability.

• Nuclear power plants use the process of nuclear fission to produce heat in nuclear reactors.

Applications of

Nuclear Fission

Nuclear Fusion

• The third type of nuclear reaction is fusion, which is the combining of atomic nuclei.

• Fusion reactions can release very large amounts of energy but require extremely high temperatures.

Nuclear Fusion

• For example, nuclear fusion occurs within the Sun, where hydrogen atoms fuse to form helium atoms.

20. What is the main difference between nuclear fusion and nuclear fission?

Question

Nuclear fusion is the combining of nuclei to form a single nucleus. Nuclear fission is the splitting of a nucleus into fragments.

nuclear chemistry element# of neutrons # of protons # of electrons atomic # mass # scan- dium iron n...

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